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11 Cards in this Set
- Front
- Back
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Equilibrium
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- Rate of forward and reverse reactions are the same
- Can be measured through equilibrium constant (Keq) |
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Keq (Equilibrium Constant)
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- [Products]/[Reactants]
- No pure liquids or solids in expression - Can use partial pressures and concentrations - Only valid at one temperature |
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What if Keq > 1?
What if Keq < 1? |
- If > 1, then products is greater than reactants and are favored at equilibrium
- If < 1, then reactants are favored at equilibrium |
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Reaction Quotient (Q)
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- Expression for a reaction that is NOT in equilibrium
- [Products]/[Reactants] Q ----> Keq <---- Q - If less than Keq, reaction goes in the forward direction to reach equilibrium - If greater than Keq, reaction goes in the reverse direction to reach equilibrium |
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Le Chatlier's Principle
STRESSORS |
- Temperature
- Pressure and Volume - Change in reactants or products |
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Le Chatlier's Principle
NON-STRESSORS |
- Inert Gas
- Catalyst |
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Le Chatlier's Principle
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- A system at equilibrium will try to neutralize any change to maintain the system at equilibrium
- If it's temp or heat, treat as product/reactant - If it's volume, consider # of mols |
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Solubility Product Constant (Ksp)
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- Dissolution of salts and the extent of which they can dissolve in water
- [Products]/[Reactants] - Pure solids don't go in reaction equation - The higher the Ksp, the more soluble the salt. |
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Ion Product Constant (Qsp)
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- Same thing, just not at equilibrium. Compare to Keq and Q.
Qsp ----> Ksp <---- Qsp - If Qsp > Ksp, then excess salts will precipitate. - If Qsp < Ksp, more stuff can still dissolve. - If the two are equal the solution is "SATURATED" |
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Molar Solubility
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- Tells how many moles of a solt can dissolve in 1L of a solution using either Ksp or Qsp
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Common Ion Effect
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- Decrease in solubility of a salt when you add the salt to a solution that is a source for one of the ions
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